Neutralization rxns and Titration of strong acid
titration curves with strong base
- titration: commonly used in acid
- remember: story acids/
base neutralization rxns to
bases ionize completely
determine the amount of aid or
in water. The h3o+ from
base in a solution.
acid and oh- from base
- involved solution of known
react
concentration (titrant)
- h30+ + oh- —> 2h2o
delivered from a buret into
- must do Stoichiometry to
an unknown solution until
find equivalence point!
substance being analyzed is
(Volume of the base in
consumed
ml). see pic below.
- stoichiometric/equivalence point:
- initial ph
the point in an acid-base
- ph at this point is
titration when the equivalents
calculated from
of a base equal to the
concentration of the
equivalents of acid
acid
- number of moles of base =
- use regular -log
number moles of acid
equation to solve:
- end point: point in titration
pH log [Acid ]
= -
where indicator changes color
- Ph after adding 5.0ml of
- goal is to choose an
base
indicator such that the
- ph calculated from
indicator changes color
unreacted hcl. Calculate
within the ph range of the
[h3o+] by using
solution at the equivalence
stoichiometric table. (See
point
pic below)
- an indicator is used to signal
- at equivalence point
end point.
- when amount of
- added at beginning of
titration at equivalence
titration that changes
point is added, all the
color at or very near
h3o+ and oh- have
equivalence point
reacted to form water.
, - millimole: often easier to work - only sources for h3o+
with millimoles and ml than and oh- are from
moles and liter autoionization of water
- ph = 7
M =
Mol OR M=Mmol
ML PH -10g 1.00 x 10"
= =7.00
- After equivalence point
- during titration, ph of the - ph calculated from
solution being titratEd excess oh- from the
changes with the addition of base. Use stoichiometric
titrant table. (See pic below)
- when ph of solution at
different stages during a
titration is plotted against
volume of titrant added, we
get a titration curve
Titration of weak acid and
strong base
- remember: the weak acid (which
ionizes very little) reacts with
the oh- from the strong base
(which ionized completely
- find equivalence point from this
(see pic below)
- Initial ph
- ph from here is calculated from
weak acid. Use ice table
- ph after 5.0ml of base
- when titrations a weak acid and
strong base, the added strong
base converts some of the acid
into its conjugate base, making
it a buffer.
- use Henderson-hasselbalch
titration curves with strong base
- titration: commonly used in acid
- remember: story acids/
base neutralization rxns to
bases ionize completely
determine the amount of aid or
in water. The h3o+ from
base in a solution.
acid and oh- from base
- involved solution of known
react
concentration (titrant)
- h30+ + oh- —> 2h2o
delivered from a buret into
- must do Stoichiometry to
an unknown solution until
find equivalence point!
substance being analyzed is
(Volume of the base in
consumed
ml). see pic below.
- stoichiometric/equivalence point:
- initial ph
the point in an acid-base
- ph at this point is
titration when the equivalents
calculated from
of a base equal to the
concentration of the
equivalents of acid
acid
- number of moles of base =
- use regular -log
number moles of acid
equation to solve:
- end point: point in titration
pH log [Acid ]
= -
where indicator changes color
- Ph after adding 5.0ml of
- goal is to choose an
base
indicator such that the
- ph calculated from
indicator changes color
unreacted hcl. Calculate
within the ph range of the
[h3o+] by using
solution at the equivalence
stoichiometric table. (See
point
pic below)
- an indicator is used to signal
- at equivalence point
end point.
- when amount of
- added at beginning of
titration at equivalence
titration that changes
point is added, all the
color at or very near
h3o+ and oh- have
equivalence point
reacted to form water.
, - millimole: often easier to work - only sources for h3o+
with millimoles and ml than and oh- are from
moles and liter autoionization of water
- ph = 7
M =
Mol OR M=Mmol
ML PH -10g 1.00 x 10"
= =7.00
- After equivalence point
- during titration, ph of the - ph calculated from
solution being titratEd excess oh- from the
changes with the addition of base. Use stoichiometric
titrant table. (See pic below)
- when ph of solution at
different stages during a
titration is plotted against
volume of titrant added, we
get a titration curve
Titration of weak acid and
strong base
- remember: the weak acid (which
ionizes very little) reacts with
the oh- from the strong base
(which ionized completely
- find equivalence point from this
(see pic below)
- Initial ph
- ph from here is calculated from
weak acid. Use ice table
- ph after 5.0ml of base
- when titrations a weak acid and
strong base, the added strong
base converts some of the acid
into its conjugate base, making
it a buffer.
- use Henderson-hasselbalch
